Antimony pentasulfide is an inorganic compound of antimony and sulfur, also known as antimony red. It is a nonstoichiometric compound with a variable composition. Its structure is unknown.[2] Commercial samples are contaminated with sulfur, which may be removed by washing with carbon disulfide in a Soxhlet extractor.

Antimony pentasulfide
Names
Other names
Antimony red
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.013.869 Edit this at Wikidata
EC Number
  • 215-255-5
UNII
  • InChI=1S/5S.2Sb checkY
    Key: PPKVREKQVQREQD-UHFFFAOYSA-N checkY
  • S=[Sb](=S)S[Sb](=S)=S
Properties
Sb2S5
Molar mass 403.82 g·mol−1
Appearance Red powder
Density 4.12 g/cm 3
Melting point 135 °C (275 °F; 408 K) (decomposes)
insoluble
Solubility soluble in HCl, alkalis, ammonium hydrosulfide
Pharmacology
R05CA07 (WHO)
Hazards
GHS labelling:
GHS02: FlammableGHS07: Exclamation markGHS09: Environmental hazard
Warning
H228, H302, H332, H411
P210, P240, P241, P261, P264, P270, P271, P273, P280, P301+P312, P304+P312, P304+P340, P312, P330, P370+P378, P391, P501
Flash point flammable
NIOSH (US health exposure limits):
PEL (Permissible)
TWA 0.5 mg/m3 (as Sb)[1]
REL (Recommended)
TWA 0.5 mg/m3 (as Sb)[1]
Related compounds
Related compounds
Antimony(III) sulfide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Production

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Antimony pentasulfide can be produced by the reaction of antimony with sulfur at a temperature from 250 to 400 °C in an inert atmosphere.

Uses

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It may be used as a red pigment and is one possible precursor to Schlippe's salt, Na3SbS4·9H2O, which can be prepared according to the equation:

3 Na2S + Sb2S5 + 9 H2O → 2 Na3SbS4·9H2O

It is also used in the vulcanization of rubber to produce red rubber.

Physical chemistry

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Like many sulfides, this compound liberates hydrogen sulfide upon treatment with strong acids such as hydrochloric acid.[3]

6 HCl + Sb2S5 → 2 SbCl3 + 3 H2S + 2 S

Analysis by Mössbauer spectroscopy indicates that this compound is a derivative antimony(III),[4] explaining the production of antimony(III) chloride, rather than antimony(V) chloride, upon acidification. It is, therefore, not analogous to the phosphorus(V) compound phosphorus pentasulfide.

References

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  1. ^ a b NIOSH Pocket Guide to Chemical Hazards. "#0036". National Institute for Occupational Safety and Health (NIOSH).
  2. ^ Arnold F. Holleman, Nils Wiberg: Lehrbuch der Anorganischen Chemie, 102nd edition, de Gruyter, Berlin 2007, p. 849, ISBN 978-3-11-017770-1.
  3. ^ Strem MSDS
  4. ^ G. G. Long; J. G. Stevens; L. H. Bowen; S. L. Ruby (1969). "The oxidation number of antimony in antimony pentasulfide". Inorganic and Nuclear Chemistry Letters. 5 (1): 21–25. doi:10.1016/0020-1650(69)80231-X.